|Publication number||US7537747 B2|
|Application number||US 10/860,628|
|Publication date||May 26, 2009|
|Filing date||Jun 3, 2004|
|Priority date||Jun 3, 2004|
|Also published as||US20050271581|
|Publication number||10860628, 860628, US 7537747 B2, US 7537747B2, US-B2-7537747, US7537747 B2, US7537747B2|
|Inventors||Martin S Meyer, Frederick E Pinkerton, Gregory P Meisner|
|Original Assignee||Gm Global Technology Operations, Inc.|
|Export Citation||BiBTeX, EndNote, RefMan|
|Patent Citations (27), Non-Patent Citations (28), Referenced by (3), Classifications (20), Legal Events (14)|
|External Links: USPTO, USPTO Assignment, Espacenet|
The present invention relates to hydrogen storage, the methods and compositions.
Hydrogen is desirable as a source of energy because it burns cleanly in air producing water as a by-product. In order to enhance the desirability of hydrogen as a fuel source, particularly for mobile applications, it is desirable to increase the available hydrogen content per unit volume of storage. Presently, this is done by conventional means such as storage under high pressure, at thousands of pounds per square inch, cooling to a liquid state, or absorbing into a solid such as a metal hydride. Pressurization and liquification require relatively expensive processing and storage equipment.
Storing hydrogen in a solid material such as metal hydrides, provides volumetric hydrogen density which is relatively high and compact as a storage medium. Binding the hydrogen as a solid is desirable since it desorbs when heat is applied, thereby providing controllable desorption.
Rechargeable hydrogen storage devices have been proposed to facilitate the use of hydrogen. Such devices may be relatively simple and generally are simply constructed as a shell and tube heat exchanger where the heat transfer medium delivers heat for desorption. Such heat transfer medium is supplied in channels separate from the chamber which houses the hydrogen storage material. Therefore, when hydrogen release is desired, hot fluid may be circulated through the channels, in heat transfer relationship with the storage material, to facilitate release of the hydrogen. To recharge the storage medium, hydrogen may be pumped into the chamber and flow through the storage material while the heat transfer medium removes heat, thus facilitating the charging or hydrogenating process. An exemplary hydrogen storage material and storage device arranged to provide suitable heat transfer surface and heat transfer medium for temperature management is exemplified in U.S. Pat. No. 6,015,041.
Presently, magnesium and magnesium-based alloys are considered to be the highest capacity hydrogen storage material with some reversible performance. However, there is limitation in that such magnesium based materials take up hydrogen at very high temperature and high hydrogen pressure. In addition, hydrogenation of the storage material is typically impeded by surface oxidation of the magnesium.
Therefore, in response to the desire for an improved hydrogen storage system, the present invention provides an improved hydrogen system, composition, and method of operation.
It is undesirable to expose fuel cell catalyst to ammonia. Ammonia present in hydrogen feed gas to the fuel cell, even at very low concentrations is undesirable. Ammonia is quite chemically reactive and may degrade other components of the hydrogen fuel system, aside from the fuel cell itself.
By the present invention there is provided systems and methods for mitigating, preventing, or at least counteracting to some extent, the production of ammonia. It has been determined that the addition of nitrogen to the atmosphere in contact with the hydrogen storage material suppresses ammonia production and contributes to causing the equilibrium of reaction to be driven in the desirable direction; that is, not favoring ammonia formation.
Accordingly, any amount of nitrogen by volume in the system is beneficial. In the system, as hydrogen is added to the metal-nitrogen compound (exemplary imide) to form the hydrogenated metal-nitrogen compound (exemplary amide), it is desirable to have some amount of nitrogen present along with the hydrogen in the atmosphere to counteract decomposition of the metal-nitrogen hydrogenated compound (amide) as it is formed during uptake of hydrogen by the metal-nitrogen compound (imide). In the exemplary amide/imide system, once the system is hydrogenated or hydrided, and essentially all of the imide has reacted with hydrogen to form an amide, it is desirable to maintain the amide/hydride storage material in an atmosphere that comprises nitrogen. Further, upon cycling of the amide/hydride storage material to release hydrogen, it is desirable to maintain such material in a nitrogen-containing atmosphere during dehydriding or dehydrogenation, as hydrogen is evolved therefrom. In the case where the hydrogenated material is held under the nitrogen-containing atmosphere and in the case where the hydrogen-containing material is cycled to release hydrogen therefrom, the nitrogen-containing atmosphere may also desirably comprise any inert gas, such as helium and argon. The term “inert” refers to any gas that does not participate in or affect the hydrogen storage reaction; that is, hydriding or dehydriding.
Therefore, such atmosphere may comprise nitrogen alone, or nitrogen in combination with other gasses such as hydrogen or helium. By the present work, it was recognized for the first time that decomposition of the amide is problematic and will continue until essentially all the amide is consumed, rendering the hydrogen storage material essentially effectively useless.
In the present invention, various compositions containing nitrogen were explored, including nitrogen-containing systems having a small amount of nitrogen greater than zero volume percent nitrogen or having some amount of nitrogen present in the system and up to 100% nitrogen, except in the case where hydrogen is desirable to be included in the atmosphere in order to achieve hydriding or hydrogenation. In cases where hydriding or hydrogenation is undertaken, hydrogen will be present in the atmosphere in compositions containing hydrogen including up to just under 100 volume percent hydrogen and having nitrogen present. A 50/50 volume percent hydrogen and nitrogen system is practical for use with a fuel cell.
In another aspect, the invention provides a hydrogen storage system utilizing a H2 storage medium having a hydrogenated state and a dehydrogenated state. In a preferred system, such medium comprises a hydrogenated metal-nitrogen compound such as an amide in the hydrogenated state; most preferably, such composition comprises an amide and a hydride. The amide is preferably represented by the general formula MId[(NH2)−1]d and the hydride is preferably represented by the general formula MIIf Hf, where MI and MII respectively represent cationic species or a mixture of cationic species other than hydrogen, and d and f respectively represent the average valence states.
In a dehydrogenated state, the medium comprises a metal-nitrogen compound such as an imide, which is represented by the formula Mc[(NH)−2]c/2, where M represents at least one cationic species other than hydrogen and c represents the average valence state of M.
In the method of the invention of hydrogen storage, storage is accomplished with a gaseous mixture comprising N2 and H2. According to the present invention, a gaseous mixture comprising hydrogen gas and N2 gas is contacted with the metal-nitrogen compound, such as the imide having one or more cations besides hydrogen, and upon uptake of hydrogen forms at least two distinct compounds different from the imide namely, the amide and one other compound, preferably the hydride.
As the imide takes up hydrogen for storage therein, heat is released and the aforesaid amide is formed. Thus, the imide is an exothermic hydrogen absorber. However, in a competing reaction, such as in the case of an exemplary amide, two atomic units of amide combine to release NH3 and reform the imide. This competitive reaction is undesirable and the presence of N2 mitigates occurrence of such competing reaction.
The N2/H2 mixture permits H2 uptake while not promoting NH3 formation as is the case in equivalent conditions under H2 atmosphere at the same temperature and pressure. This preserves the hydrogenated metal-nitrogen compound such as amide for use in the reverse reaction. Thus, when the hydrogenated compound such as amide and the hydride release hydrogen in the presence of one another, driven by heat, and the imide is formed, decomposition of amide is avoided. Accordingly, heat is used to cause the amide and the hydride to desorb or release hydrogen, and this reaction is endothermic. The extent of this reaction is related to the mass of sorbent amide material available. Thus the mitigation of NH3 formation is desirable.
As used herein, the term “metal-nitrogen compound” also encompasses metalloid-nitrogen compounds.
Further areas of applicability of the present invention will become apparent from the detailed description provided hereinafter. It should be understood that the detailed description and specific examples, while indicating the preferred embodiment of the invention, are intended for purposes of illustration only and are not intended to limit the scope of the invention.
The present invention will become more fully understood from the detailed description and the accompanying drawings, wherein:
The following description of the preferred embodiment(s) is merely exemplary in nature and is in no way intended to limit the invention, its application, or uses.
In one aspect, the nitrogen-containing atmosphere of the invention is utilized in an exemplary hydrogen storage system having a hydrogenated state and a dehydrogenated state, therein providing two distinct physical states where hydrogen can be stored and subsequently released. In the hydrogenated state, such composition comprises an exemplary amide and a hydride, each of which are solids. The amide is preferably represented by the general formula MId[(NH2)−1]d and the hydride is preferably represented by the general formula MIIf Hf, where MI and MII respectively represent cationic species or a mixture of cationic species other than hydrogen, and d and f respectively represent the average valence states.
In a dehydrogenated state, the composition comprises an imide, which is a solid and is represented by the formula Mc[(NH)−2]c/2, where M represents at least one cationic species other than hydrogen and c represents the average valence state of M.
In one aspect of the method of hydrogen storage of the present invention, a gaseous mixture comprising nitrogen and hydrogen is contacted with the imide having such one or more cations besides hydrogen, and upon uptake of hydrogen, forms at least two distinct compounds different from the imide namely, the amide and the hydride. This corresponds to the hydrogenated state for the storage material. The nitrogen and hydrogen-containing atmosphere leads to lessened formation of NH3 (ammonia) as compared to an atmosphere which does not contain nitrogen.
A preferred imide is lithium imide represented by the formula Li2NH, wherein the cation species is lithium, and the preferred distinct compounds formed upon hydrogen uptake are the amide represented by formula LiNH2, and the hydride represented by the formula LiH. The tendency for decomposition of 2 molecular units of LiNH2 (amide) to form Li2NH (imide) and ammonia (NH3) is lessened.
In the absence of nitrogen, decomposition by producing NH3 will occur any time the hydrogen storage material is at elevated temperature greater than about 155° C. and the material is in the hydrided state, or even a partially hydrided state. It only requires that some LiNH2 be present in order to have the source material for the decomposition reaction. Therefore, for effective suppression it is necessary for N2 to be present any time the sample is at elevated temperature. The only exception is when the sample has been completely dehydrided—then the sample cannot decompose because there is no LiNH2. In practice in a real system, this will never be the case (it amounts to running the tank completely dry, to use the gasoline equivalent). In a real system, it is desirable for N2 to always be present.
In a hydrogenated state, or while hydrogen is being released, decomposition will occur even in an inert atmosphere such as pure He. For example, experimental data on the system LiNH2+LiH shows that the amount of weight loss (5.2 wt %) during dehydriding in 130 kPa He gas at 240° C. is greater than the amount of weight gain (4.7 wt %) during the subsequent hydriding in a mixture of 50% H2/50% N2 gas at 260 kPa and 230° C. The extra weight represents the NH3 lost during dehydriding in pure He. At elevated temperature, there is weight loss both due to H2 removal and due to NH3 removal. The weight loss stops in pure He once the sample is fully dehydrided, but that is because the surviving hydrogen storage portion of the sample has been fully converted to Li2NH and there is no more LiNH2 in the sample to decompose.
Referring back to the exemplary systems of the invention, it should be understood that in the present invention M, MI and MII each represent a cationic species or mixture of cationic species other than hydrogen. Examples are metal cations, non-metal cations such as boron, and non-metal cations which are organic such as CH3. Elements that form preferred amides, imides, hydride-nitrides, and mixtures of cations in the type of compounds of the present invention are as follows. For amides the cationic species comprise: Li, Be, Na, Mg, K, Ca, Ni, Rb, Sr, In, Cs, Ba, La, Sm, Eu, and Yb. For imides the cationic species comprise: Li, Na, Mg, Ca, Sr, Ba, La, Eu, and Th. For hydride-nitride the cationic species comprise: Si, Ca, Ti, Sr, Zr, Ba, and Th. For mixed amide/imide the cationic species comprise: Li, Be, Na, Mg, Al, Si, K, Ca, Mn, Zn, Ga, Rb, Sr, Y, In, Sn, Cs, Ba, La, Pb, Ce, Nd, Sm, Eu, Gd, and Yb. For other related materials such as coordination-type NH-containing materials the cationic species comprise: Li, Be, B, Na, K, Ca, Ni, Cu, As, Se, Sr, In, Sb, La, W, Eu, and Th. Evaluation of the aforesaid known species produces, by analogy the following added cationic species besides those recited above which are thought to be usable but not yet demonstrated, include Fe, Sc, Ge, Cd, Hf, Hg, TI, and Pr. In view of the above, the cationic species generally comprise: aluminum (Al), arsenic (As), boron (B), barium (Ba), beryllium (Be), calcium (Ca), cadmium (Cd), cerium (Ce), cesium (Cs), copper (Cu), europium (Eu), iron (Fe), gallium (Ga), gadolinium (Gd), germanium (Ge), hafnium (Hf), mercury (Hg), indium (In), potassium (K), lanthanum (La), lithium (Li), magnesium (Mg), manganese (Mn), sodium (Na), neodymium (Nd), nickel (Ni), lead (Pb), praseodymium (Pr), rubidium (Rb), antimony (Sb), scandium (Sc), selenium (Se), silicon (Si), samarium (Sm), tin (Sn), strontium (Sr), thorium (Th), titanium (Ti), thallium (TI), tungsten (W), yttrium (Y), ytterbium (Yb), zinc (Zn), and zirconium (Zr).
An analysis of the behavior and crystallography of the aforesaid amides, imides, hydride/nitride, mixed amide/imide, and other related materials such as coordination-type NH-containing materials reveals that some of the aforesaid compounds such as lithium demonstrate a relatively simple chemistry of the amide and the imide. Other materials, particularly hydride/nitride compounds involving calcium and relatively heavier cation elements, form related phases based upon systematic behavior demonstrated by the imides and amides and according to the literature. Such related materials are not necessarily characterized as an amide or an imide and principally fall into the category of the hydride/nitride stated earlier. Such materials involve hydrogen and nitrogen and comprise cationic species and ammonia complexes, so they are ammonia-containing materials, but not amides or imides. Such more complex type salts involve the aforesaid cations having a higher number of nitrogen surrounding it as compared to the amide and imides. For example, simple lithium amide has an Li coordinated with one NH2. Whereas, the more complex compounds have the lithium coordinated with more than one NH3 group. Therefore, the invention encompasses all of the hydrogen storage capable nitride/hydride type materials and compounds some of which involve cations having affinity to ammonia as well as the more traditional NH2. The invention also contemplates intermediate products arising during a series of reactions in the gas and solid phases associated with the hydrogen storage media.
It should be noted that M, MI and MII are independently selected and each may be different, or any two or more may be the same, cationic species. Preferably M, MI and MII each represent one or a mixture selected from the group consisting of lithium, magnesium, sodium, boron, aluminum, beryllium, and zinc. In a preferred embodiment, all such M, MI and MII represent lithium, or mixed metal including lithium, such as LiNa.
As the imide takes up hydrogen for storage therein, heat is released and the aforesaid amide and hydride are formed. Thus, the imide is an exothermic hydrogen absorber. In the reverse reaction, the amide and hydride release hydrogen in the presence of one another, driven by heat, and the imide is formed. Accordingly, heat is used to cause the amide and the hydride to desorb or release hydrogen.
Preferred temperature and pressure conditions for charging the hydrogen into the storage material are temperatures in a range from about room temperature to about 380° C. and H2 pressures from about 0 (vacuum) to about 1000 kPa. At about 380° C. and less than about 1000 kPa H2 pressure, hydrogen will tend to be released. At lower temperatures the H2 pressure to release is correspondingly lower.
It should be noted that the system behaves in a manner whereby at each temperature, there is a threshold H2 pressure above which hydrogen is absorbed and below which hydrogen is desorbed. For example, at 125° C. in order to desorb, the H2 pressure is preferably less than 10 kPa. It is possible to desorb hydrogen at H2 pressures less than about 1000 kPa at temperatures higher than about 340° C. By way of further example, at room temperature, the H2 pressure for hydrogen release is near zero, vacuum. At elevated temperatures, on the order of 380° C., hydrogen is released until an H2 pressure above about 1000 kPa is reached. Then at such sufficiently elevated pressure, hydrogen is inserted. The term “H2 pressure” is used to distinguished from the overall pressure of the gas mixtures. The cycling of H2 is related to and depends on the hydrogen pressure, and is relatively independent of the total pressure of a mixed gas.
Particle size of the storage material is related to its performance. Particles that are too coarse extend the time for absorption/desorption at a given temperature. It has been found that starting material particle size on the order of 500 microns (one half millimeter) ball milled for 1 to 10 hours form suitable material. This results in particle size on the order of less than about 10 microns.
In still another aspect of the invention, there is provided a method for forming the imide based hydrogen storage material which comprises reacting the amide in the presence of the hydride to form the imide storage medium. Here, the amide and hydride in particulate form are mixed together and heated to release hydrogen and form the imide product, under atmosphere containing nitrogen.
The foregoing lithium storage system based upon the imide absorbs hydrogen at a temperature of preferably greater than or equal to 145° C. and hydrogen pressures as low as 5 kPa, but preferably greater than or equal to 15 kPa. In a preferred system, the amide and hydride constituents release or desorb hydrogen at a temperature greater than or equal to 125° C. and at hydrogen pressure that is less than or equal to 10 kPa, thereby forming the imide constituent as heretofore described.
Use of the nitrogen and hydrogen-containing atmosphere which leads to lessened formation of NH3 (ammonia) as compared to an atmosphere which does not contain nitrogen, will now be further explained by reference to examples. In these examples, the tendency for irreversible decomposition of amide to form ammonia in the absence of nitrogen is shown for the various species and genus as described herein as exemplified by the Li species. The beneficial effect of nitrogen is also clearly demonstrated.
In use, the invention relates to the reversible hydrogen storage reaction given by:
In the hydrided state, LiNH2 can also irreversibly decompose at temperatures greater than 155° C. according to:
2 LiNH2→Li2NH+NH3. (2)
Thus the hydrided material will readily decompose by releasing ammonia at the operating temperature of the hydriding/dehydriding (hydrogenating/dehydrogenating) reaction (≧175° C.). In the presence of hydrogen gas, the combined effect of reactions (1) and (2) is to completely convert the material over time to LiH and ammonia gas, thereby destroying its ability to store and release hydrogen.
Adding nitrogen gas to the working atmosphere inhibited ammonia production. Initial experiments used a gas mixture containing 8% H2 and 92% N2, which constitutes a very nitrogen-rich mixture. Good results were obtained. In order to further examine the effect of nitrogen concentration on ammonia suppression, the inhibitory effects of a 50% H2/50% N2 mixture were compared to both pure H2 gas and to a nitrogen-rich 5% H2/95% N2 mixture in the examples below. The 50% N2 mixture also provides ammonia inhibition, and the data suggest that ammonia inhibition improves with increasing N2 concentration. Accordingly, any amount of nitrogen present in the atmosphere is beneficial, with the extent of benefit increasing with increasing nitrogen.
LiNH2+LiH hydrogen storage materials were prepared by combining stoichiometric quantities of the two starting compounds, LiNH2 and LiH, in a hardened steel ball mill jar along with one large and two small steel milling balls. The total weight of the mixed powder was 1 gram. In order to protect the material from air exposure, the jar was loaded and sealed under an Ar inert gas atmosphere inside of a glove box. The mixed material was then ball milled for 10 hours using a SPEX 8000 Mixer/Mill in order to reduce the particle size and to intimately mix the two constituents. Several such 1 gram batches were prepared in the course of the experiments.
Hydrogen release and ammonia production were evaluated using a Cahn Model 2151 high-pressure thermogravimetric analyzer (TGA). The weight of the sample was monitored as it was heated in a hydrogen or mixed hydrogen-nitrogen atmosphere. Release of either hydrogen or ammonia appears as weight loss from the sample. Simultaneously, a mass spectrometer was used to perform residual gas analysis (RGA) of the gas flowing through the TGA. The RGA signal at mass 17 amu thus provided an independent measurement of the quantity of ammonia NH3 given off by the sample.
Three gas concentrations were used:
The 100% H2 (nitrogen-free) gas was the baseline case for comparison of ammonia production. Pure H2 gas was used at the minimum working gas pressure of the TGA, 130 kPa.
For each of the mixed gas concentrations, the material was tested at two different pressures. In one case, the mixed gas used was at the same pressure as the pure H2, namely 130 kPa. Alternatively, a total pressure was used that would provide a 130 kPa H2 partial pressure; i.e., 260 kPa for the 50% H2 mixture and 2600 kPa for the 5% H2 mixture. For these pressures the amount of hydrogen present remains constant, which helps ensure that results are due to the nitrogen gas. The experimental conditions were as in Table 1:
Experimental conditions used in ammonia suppression tests.
130 kPa H2 partial
Stepped Temperature Experiments
In these experiments the temperature was increased in 25° C. increments from 100° C. to 275° C. At each step the temperature was held constant for a period of time ranging from 100 to 200 min. As examples,
This interpretation is supported by the RGA data in
Normalized NH3 signal=mass 17 signal−0.23×mass 18 signal (3)
In addition, there is a background instrumental signal in the mass spectrometer that occurs even in the absence of NH3. This background contribution to the normalized NH3 signal is about 4×10−10 Torr at 200 min in
A similar experiment (not shown) was performed for the 50% H2/50% N2 gas mixture at 260 kPa; i.e., at the same H2 partial pressure of 130 kPa. The results are shown as the solid triangles in
The weight measurements for the 100% H2 and 50% H2 gas mixtures had very low noise levels. In contrast, the 5% H2/95% N2 mixture at 2600 kPa has considerably greater noise, as shown in
In summary, the stepped temperature experiments show the following features: (1) NH3 generation is clearly evident in the baseline 100% H2 experiment at 130 kPa pressure, as observed in both the mass loss rate and the normalized NH3 partial pressure. Small quantities of NH3 may be produced at temperatures as low as 125° C., and unambiguous NH3 generation is evident at temperatures of 175° C. and higher. (2) The 5% H2/95% N2 mixture shows little or no NH3 production at 2600 kPa (130 kPa H2 partial pressure). The noise in the weight measurement produces uncertainty in the mass loss rate data, but to within experimental error the mass loss rate remains zero or very close to zero at all temperatures below 275° C. Of the two 5% H2 experiments, one produced RGA data indicating no production of ammonia, and the other suggests that a small amount of ammonia production may occur above 225° C. (3) For the 50% H2 mixture slight NH3 production may occur above 200-225° C. (4) Results for the gas mixtures at 130 kPa total pressure are consistent with these results.
Scanned temperature experiments
Scanned temperature experiments were also performed, wherein the sample weight and RGA signals are monitored as the temperature is continuously increased at a heating rate of 5° C./min.
The mass data are more difficult to interpret in these experiments due to the effects of temperature ramp-induced transients in the weight and the simultaneous production of H2 and NH3 at high temperature. Ammonia production is unambiguous in the RGA data in the lower panel.
Prior to the release of any gases (<40 min) all of the RGA mass signals change linearly with time due to small drifts in the background level. The dashed lines on the mass 17 and normalized NH3 curves are extrapolations of the background to longer times, showing that indeed ammonia is produced from the sample beginning at about 45 min.
Ammonia release onset times (and equivalent temperatures) were determined as follows. A 9th order polynomial fit to the normalized NH3 data was done in order to smooth the noise. The resulting fits are shown as the solid lines in
The onset times are shown in
The onset temperatures are somewhat higher than those obtained in the stepped temperature method. The trends in the data are clear—increasing the N2 concentration of the gas pushes the onset of ammonia release to higher temperatures, and decreases the quantity of ammonia released at high temperature (>280° C.), by as much as an order of magnitude in the case of 5% H2.
In summary, the stepped temperature and scanned temperature experiments show many important advantages of including N2 gas with the H2 gas atmosphere:
First, ammonia loss from LiNH2+LiH hydrogen storage material is unambiguously detectable by both mass loss and direct RGA detection at 175° C. in pure H2 gas at 130 kPa, and there is evidence for small amounts of NH3 production even as low as 125° C. Ammonia production accelerates rapidly as the temperature increases.
Second, in a 5% H2/95% N2 mixture ammonia production is inhibited. The onset of ammonia release is moved up to at least 225° C. In the stepped temperature experiments, the evidence for any ammonia release is essentially absent, even up to 275° C. If ammonia release does occur in this temperature range, the quantity of ammonia released is much smaller than for the pure H2 gas. The scanned temperature experiment shows that some ammonia release does occur at high temperature (>280° C.), but at a rate about one order of magnitude smaller than in pure H2.
Third, the intermediate case of 50% H2/50% N2 shows a small amount of ammonia release starting at temperatures of about 200° C. The amount of ammonia evolved is diminished by about an unexpectedly substantial factor of 4-5 compared to that of pure H2. Scanned temperature experiments are consistent with the interpretation that the onset temperature for NH3 release is higher than that of pure H2, but not quite as high as that of the 5% H2 mixture.
Comparing the results for 130 kPa fixed H2 partial pressure with the results for 130 kPa total pressure indicates that the H2/N2 mixture, rather than the H2 partial pressure, is responsible for these effects. Thus, clearly, the presence of nitrogen gives a very beneficial result.
Accordingly, ammonia production from LiNH2+LiH is inhibited by the addition of N2 to the H2 gas used in absorption and desorption of hydrogen. The degree of inhibition depends on the percentage of N2 gas in the mixture. The 5% H2/95% N2 mixture suppressed ammonia production completely, or nearly so, below 275° C. Inhibition by the 50% H2/50% N2 mixture was not quite as good, but still afforded a very marked increase in the onset temperature for ammonia release to about 200° C. and a very significant reduction in the rate of ammonia production at higher temperature compared to pure H2 gas.
Thus, the N2-containing atmosphere of the present invention provides reversible solid phase hydrogen storage, while reducing the evolution of NH3 as compared to a system without N2 in the atmosphere. This is especially advantageous in fuel cell applications where the presence of NH3 in the fuel cell system is undesirable. Commercial grade hydrogen for fuel cell use typically contains at least 99.995 volume % hydrogen and the balance impurities, including water, CO/CO2, and nitrogen. Glove box purifier regeneration grade hydrogen typically contains 2-10 volume % H2 80 to 95% N2 and 3-10 volume % CO2. These atmospheres are not anywhere known to be used in cycling a hydrogen storage system. Such atmospheres are useable in the present invention.
Greater N2 decreases NH3 formation and greater H2 provides the necessary H2 partial pressure for efficient fuel cell operation. For a preferred fuel cell anode feed, H2 partial pressure of 2 to 5 atmospheres, a 50/50 mix of H2/N2 is delivered at 4 to 10 atmospheres.
Since the benefit of nitrogen to offset NH3 formation is essentially proportional to the amount of N2, the ranges of hydrogen and nitrogen content are varied. In various embodiments:
The description of the invention is merely exemplary in nature and, thus, variations that do not depart from the gist of the invention are intended to be within the scope of the invention. Such variations are not to be regarded as a departure from the spirit and scope of the invention.
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|6||Goubeau, et al., "Über ternäre Metall-Bornitride", Zeitschrifte für anorganishe und allgewieine, Chemic vol. 310 (1961) 248-260.|
|7||Herbert Jacobs and Robert Juza, "Preparations and Properties of Magnesium Amide and Imide" Journal of Anorganic and General Chemistry, Band [vol.] 870 (1969) pp. 254-261. (English translation only; original German not available.).|
|8||Hu et al., "Ultrafast Reaction between LiH and NH3 during H2 Storage in Li3N"; J. Phys. Chem. A; vol. 107, No. 46 (Nov. 20, 2003) 9737-9739.|
|9||Ichikawa et al., "Mechanism of Novel Reaction for LiNH and LiH to Li2NH and H2 as a Promising Hydrogen Storage System"; J. Phys. Chem. B; vol. 108, No. 23 (May 5, 2004) 7887-7892.|
|10||Jacobs et al., "Preparations and Properties of Magnesium Amide and Imide", Journal for Anorganic and General Chemistry, Band [vol.] 870 (1969) 254-261. (English translation only; original German not available).|
|11||JCPDS X-Ray Database; pattern No. 00-007-0245-Li3AIN2.|
|12||JCPDS X-Ray Database; pattern No. 00-036-1016-beta-Mg3B2N4.|
|13||JCPDS X-Ray Database; pattern No. 00-042-0868-Mg3BN3.|
|14||JCPDS X-Ray Database; pattern No. 00-044-1497-Mg3BN3.|
|15||JCPDS X-Ray Database; pattern No. 16-273-Li3BN2.|
|16||JCPDS X-Ray Database; pattern No. 40-1166-Li3BN2.|
|17||JCPDS X-Ray Database; pattern No. 80-2274-Li3BN2.|
|18||Juza et al., "Die ternären Nitride Li3AIN2 und Li3GaN2"; Zeitschrifte für Anorganische Chemic, vol. 257 (1948) 13-25.|
|19||Juza et al., "Metal amides and metal nitrides", 25th Part, Journal for Anorganic and General Chemistry, 1951 vol. 266, 325-330. (English translation and German language document).|
|20||Pinkerton et al., "Bottling the Hydrogen Genie", The Industrial Physicist, (Feb./Mar. 2004) 20-23.|
|21||Pinkerton et al., "Hydrogen Desorption Exceeding Ten Weight Percent from the New Quaternary Hydride Li3BN2H8" ACS Publications, http://pubs.acs.org/cgi-bin/abstract.cgi/jpcbfk/2005/109/i01/abs/jp0455475.html.|
|22||Robert Juza and Karl Opp, Metal amides and metal nitrades, 25th Part 1), Journal for Anorganic and General Chemistry. 1951 Band vol. 266, pp. 325-330. (2 documents: English translation and original German.).|
|23||Villars et al., "ASM International Handbook of Ternary Alloy Phase Diagrams", AI Li N; AILi3N2 (1) Crystallographic Data (1997).|
|24||Villars et al., "ASM International Handbook of Ternary Alloy Phase Diagrams", B Li N; BLi3N2 (HT) (2) Crystallographic Data (1997).|
|25||Villars et al., "ASM International Handbook of Ternary Alloy Phase Diagrams", B Li N; BLi3N2 (LT) (2) Crystallographic Data (1997).|
|26||Villars, P., "Pearson's Handbook Desk Edition", Crystallographic Data for Intermetallic Phases, Ac-Cr2Se4Zr, vol. 1, p. 416 (1997) 771 and 776.|
|27||Yamane et al., "High- and Low-Temperature Phases of Lithium Boron Nitride, Li3BN2 Preparation, Phase Relation, Crystal Structure, and Ionic Conductivity", J. Solid State Chemistry, vol. 71, 1987) 1-11.|
|28||Yamane et al., "Structure of a New Polymorph of Lithium Boron Nitride, Li3BN2", J. Solid State Chemistry, vol. 65, (1986) 6-12.|
|Citing Patent||Filing date||Publication date||Applicant||Title|
|US7862791||Sep 14, 2005||Jan 4, 2011||Gm Global Technology Operations, Inc.||Hydrogen storage systems and compositions|
|US7927507 *||Mar 13, 2009||Apr 19, 2011||Hrl Laboratories, Llc||Hydrogen storage compositions|
|US20060090394 *||Sep 14, 2005||May 4, 2006||Torgersen Alexandra N||Hydrogen storage systems and compositions|
|U.S. Classification||423/413, 423/645, 423/647, 423/646, 423/648.1, 423/644|
|International Classification||C01B6/06, C01B3/04, C01B6/04, C01B21/092, C01B3/08, C01B3/06, C01B6/02, C01B6/24, C01B6/00|
|Cooperative Classification||C01B21/0923, Y02E60/362, C01B3/065|
|European Classification||C01B3/06C, C01B21/092B|
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